Metallic bonding

Front

What is metallic bonding?

Back

Metallic bonding is the electrostatic attraction between positively charged metal ions and delocalized electrons, which allows metals to conduct electricity and heat.

Front

What are alloys?

Back

Alloys are mixtures of two or more elements, where at least one is a metal, designed to enhance certain properties such as strength and resistance to corrosion.

Front

Why are alloys generally used to make everyday objects?

Back

Alloys are often stronger and less active than pure metals.

Front

Why are metals able to conduct electricity?

Back

The valence electrons are delocalized and are mobile (move).

Front

True or False: Metals can conduct heat.

Back

True.

Front

True or False: Metals give up electrons easily.

Back

True.

Front

What is the significance of delocalized electrons in metals?

Back

Delocalized electrons allow metals to conduct electricity and heat efficiently.

Front

How do the properties of alloys differ from pure metals?

Back

Alloys typically have improved strength, corrosion resistance, and lower reactivity compared to pure metals.

Front

What is the relationship between metallic bonding and the malleability of metals?

Back

Metallic bonding allows layers of atoms to slide over each other without breaking the bond, making metals malleable.

Front

What is the role of the electron sea model in understanding metallic bonding?

Back

The electron sea model describes how delocalized electrons form a 'sea' around metal cations, contributing to properties like conductivity and malleability.